# Shouldn't it take more energy to break CO2 compared to CO? [on hold]

I read in a book that bond dissociation energy of carbon monoxide $$(\ce{CO})$$ is $$\pu{749 kJ/mol}$$ and carbon dioxide $$(\ce{CO2})$$ is $$\pu{532 kJ/mol}.$$ Shouldn't it take twice as much energy to break $$\ce{CO2}?$$

## put on hold as off-topic by Buck Thorn, Karsten Theis, Mithoron, Jon Custer, Todd MinehardtJun 13 at 1:20

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• 532 kJ/mol times two... – Karsten Theis Jun 12 at 14:47
• I'm voting to close this question as off-topic because your question lacks context. This question needs revision before it is ready for a great answer. Please edit to include how this question came up and how you tried to answer it. This will help writing an answer that is useful for you and for others. – Karsten Theis Jun 12 at 18:20

The bond dissociation refers to each bond. Therefore, the number you cited for $$\ce{CO2}$$ is for only one of the C=O bonds.